Sulfur can have a wide range of oxidation in its compounds
-2 in H2S
0 in elementary sulfur (S8)
+4 in SO2
+6 in SO3
They could be formed by the oxidation / combustion of sulfur and nitrogen respectively
Sulfur oxides are the oxides of sulfur with oxygen in -2 oxidation state. There are two main oxides of sulfur. They are sulfur dioxide (SO2) and sulfur trioxide (SO3).
In HSO4- sulfur's oxidation state is +5.
The sulfate ion is SO42 -. The oxidation state of the sulfur is +6 (work it out!); therefore, the ion is more properly named the sulfate(VI) ion. The sulfite ion is SO32-. The oxidation state of the sulfur is +4.
elemental sulfur is not oxidised. It has to be in some sort of compound. For example, in H2S, the sulfur has an oxidation state of -2. Each hydrogen has a +1, so if they are removed, it decreases the overall charge. Remove two, and the charge is decreased by 2, making it -2.
There are s8 sulfur molecules. It shows 0 oxidation number.
The oxidation state of an individual sulfur atom in BaSo4 is +6.
The oxidation state of an individual sulfur atom in MgSO4 is +6.
This is the thiosulfate ion. Sulfur shows +6 oxidation number.
"oxidation"
+6 for sulfur in sulfates
The oxidation state of an individual sulfur atom in (SO3)2- is 4.
Since the total molecule must have zero net oxidation state and there are two oxygen atoms but only one sulfur atom, the sulfur must have oxidation state +4.
Atomic sulfur has oxidation number 0. The oxidation number of the sulfide ion is -2. During formation of a wide variety of compounds, the oxidation status of sulfur may differ from -2 to +6.
-2
+4
+6